Given the standard electrode reduction potentials: and . Determine the standard cell potential () in — Electrochemistry Chemistry Question
Question
Given the standard electrode reduction potentials: $E^\circ_{Sn^{2+}/Sn} = -0.14\text{ V}$ and $E^\circ_{Fe^{3+}/Fe^{2+}} = +0.77\text{ V}$. Determine the standard cell potential ($E^\circ_{cell}$) in Volts for a standard galvanic cell driven by the overall reaction $Sn(s) + 2Fe^{3+}(aq) \rightarrow Sn^{2+}(aq) + 2Fe^{2+}(aq)$.
💡 Solution & Explanation
The cell reaction consists of the oxidation of solid Tin ($Sn \rightarrow Sn^{2+} + 2e^-$) at the anode and the reduction of Iron(III) ($Fe^{3+} + e^- \rightarrow Fe^{2+}$) at the cathode. The standard EMF of the cell is calculated solely from reduction potentials as $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} = E^\circ_{Fe^{3+}/Fe^{2+}} - E^\circ_{Sn^{2+}/Sn} = 0.77\text{ V} - (-0.14\text{ V}) = 0.77 + 0.14 = +0.91\text{ V}$.